Name: atomic charges, bonds, and compounds
Uploaded: 2023-06-23T15:38:43.000Z
Duration: 1 min 23 s
Channel: JoVE

イオンは、電子を獲得または失った帯電した原子です。電子を失って正に帯電する原子を陽イオンと呼び、電子を獲得して負に帯電する原子を陰イオンといいます。
イオンは、神経インパルスの伝達や筋肉の収縮など、多くの生理学的プロセスに不可欠です。
分子は、電子を共有する2つ以上の原子の組み合わせです。それらは、酸素分子のような1つの元素の原子、または水分子のような異なる元素の原子で構成されている場合があります。
化合物とは、電子が移動しているか共有されているかに関係なく、一定の割合で化学結合した異なる元素の原子の組み合わせです。
イオン性化合物は、通常の食卓塩と同様に、金属イオンと非金属イオンの間の静電相互作用によって形成され、ナトリウムカチオンと塩化アニオンが静電相互作用を介して結合します。
分子化合物は、非金属原子が共有結合を介して結合することで形成されます。例えば、メタンは、4つの水素原子が特定の割合で炭素原子と電子を共有している分子化合物です。

イオン、分子、および化合物

イオン - 元素が1つ以上の電子を寄付または受け入れる化学反応に参加すると、元素は正または負に帯電します。ほとんどの元素では、完全な価電子殻を持つために、これが頻繁に起こります。これは、半分以上の殻を埋めるために電子を獲得して起こることもあり、半分以上の殻を空にするために電子を与えることで、次に小さい電子殻が新しい完全な価電子殻となります。電荷を持つ原子—正または負—はイオンと呼ばれます。 例えば、カリウム（K）は全ての体細胞で重要な元素です。その原子番号は19です。その価電子殻にはたった1つの電子があります。この特性により、カリウムは、1つの電子を寄付する化学反応に参加する可能性が非常に高くなります。電子の損失により、カリウムの陽性の電荷はカリウムの電子の陰性の電荷よりも影響力が強くなります。言い換えれば、結果として得られるカリウムイオンはわずかに陽性になります。陽性の電荷を持つイオンはカチオンとして知られています。 また、骨や歯の構成要素であるフッ素（F）は、原子番号9を持っています。その価電子殻には7つの電子があります。フッ素は、1つの電子を受け入れるという形で他の原子と結合する可能性が非常に高いです。そうすると、電子は陽子よりも1つ多くなり、全体的に負の電荷を持つことになります。負の電荷を持つイオンはアニオンとして知られています。 イオンは正常な体の機能にとって重要であり、そのバランスの崩れは健康問題を引き起こす可能性があります。たとえば、ナトリウムイオンのバランスの崩れは心血管疾患を引き起こす可能性があります。低い血液中のカルシウムレベルはテタニー — 制御不能な無意識の筋収縮を引き起こす可能性があります。 分子 - 分子は単に2つ以上の原子が化学的に結合したものです。分子は、酸素原子間の結合によって形成される酸素ガスの分子のように、同じ元素の原子から構成される場合もあります。また、酸素原子と炭素原子の間で形成される二酸化炭素ガスの分子のように、異なる元素の原子との間で結合が形成される場合もあります。 化合物 - 化合物は、一定比率で2つ以上の原子が結合した純粋な物質です。例えば、グルコースという化合物は重要な体の燃料です。それは常に同じ3つの元素（炭素、水素、酸素）で構成されており、同じ相対量が存在します。グルコースには常に炭素と酸素の単位が6つずつあり、水素の単位が12つあります。 このテキストは <a href="https://openstax.org/books/anatomy-and-physiology-2e/pages/2-2-chemical-bonds?query=when%20a%20atom%20participates&target=%7B%22type%22%3A%22search%22%2C%22index%22%3A0%7D#fs-id2113058">Openstax, Anatomy and Physiology 2e, Section 2.2 Chemical Bonds</a> とOpenstax, <a href="https://openstax.org/books/anatomy-and-physiology-2e/pages/2-1-elements-and-atoms-the-building-blocks-of-matter?query=For%20example%2C%20the%20compound%20glucose%20is%20an%20important%20body%20fuel.%20It%20is%20always%20composed%20of%20the%20same%20three%20elements&target=%7B%22type%22%3A%22search%22%2C%22index%22%3A0%7D#fs-id1882474">Anatomy and Physiology 2e, Section 2.1 Elements and Atoms: The Building Blocks of Matter</a>から部分的に適応されています。

イオン - 原子が化学反応に関与し、その結果、1つ以上の電子が供与または受け入れられると、原子は正になります...

Education

JoVE Core

Anatomy and Physiology

解剖生理学

Unit 1

ユニット1

Fundamentals of Chemistry

化学の基礎

KEY TERMS AND CONCEPTS

主要用語と概念

Ions, Molecules, and Compounds

atomic charges, bonds, and compounds

Atoms can gain or lose electrons during chemical reactions and become ions. An ion is an atom with an electrical charge. This charge is positive or negative, and it often helps the atom reach a full valence shell.

Some atoms are more likely to donate electrons, while others are more likely to accept them. Potassium is one example. It has atomic number 19 and one electron in its valence shell, so it is likely to donate that electron and become a slightly positive ion called a cation. Fluorine is another example. It has atomic number 9 and seven electrons in its valence shell, so it is likely to accept one electron and become a negatively charged ion called an anion.

Ions are important for normal body function, so an imbalance can cause health problems. A sodium ion imbalance can contribute to cardiovascular diseases. Low blood calcium levels can also cause tetany, which is marked by uncontrollable involuntary muscle contractions.

Molecules and compounds are related but not the same. A molecule is two or more atoms chemically bonded together. The atoms may be the same element, as in oxygen gas, or different elements, as in carbon dioxide gas. A compound is a pure substance made when two or more atoms bond in a fixed proportion.

Glucose is a useful example of a compound. It is an important body fuel and always contains the same elements in the same relative amounts: carbon, hydrogen, and oxygen. In glucose, there are always six carbon units and six oxygen units for every twelve hydrogen units.

Atomic Charges, Bonds, and Compounds

what is matter?

Matter, Mass, and Weight Basics

Matter is the substance that makes up the universe, from a grain of sand to a star. Scientists define matter as anything that occupies space and has mass. Mass is the amount of matter in an object, while weight depends on gravity. Mass stays the same whether an object is on Earth or in the zero-gravity environment of outer space. Weight changes when gravity changes. An object weighs more where gravity is stronger and less where gravity is weaker. A piece of cheese that weighs a pound on Earth...

the periodic table and organismal elements

the-periodic-table-and-organismal-elements

Organismal Elements in the Periodic Table

The periodic table helps identify the elements that make up living organisms. Biology groups these as organismal elements because they are the chemical building blocks of life. These elements are found in different amounts in the body. Some are present in large quantities, while others are needed only in small amounts. The video connects the periodic table to the elements that organisms actually use. Understanding organismal elements helps students link chemistry to biology. It shows how...

atomic structure

From Atomos to the Modern Atom

Atoms are the tiny building blocks of matter, and ideas about them go back to the Greek philosopher Democritus. He suggested that everything on Earth is made of atomos, a Greek word meaning "indivisible." That idea later led to the modern word atom. In the 19th century, John Dalton developed an atomic theory that is still largely correct today. He proposed five key ideas. All matter is made of tiny particles called atoms. Atoms of the same element are alike, and atoms of different elements are...

chemical symbols

Chemical Symbols and Element Names

Chemical symbols are short abbreviations that stand for an element or a single atom of that element. Mercury, for example, has the symbol Hg. The same symbol can point to one atom of mercury in the microscopic domain or to a sample labeled as many atoms of mercury in the macroscopic domain. Many symbols come from the element’s common name. Others are shortened from a name in another language. Most chemical symbols use one or two letters. For a few elements with atomic numbers above 112,...

atomic number and mass number

Atomic Identity, Mass, and Isotopes

Atomic identity depends on the number of protons in the nucleus, and mass depends on protons and neutrons together. The number of protons is the atomic number, or Z. It defines the element. For example, any atom with six protons is carbon, no matter how many neutrons or electrons it has. In a neutral atom, the number of protons equals the number of electrons. Because of that, the atomic number also tells you the number of electrons in the atom. The total number of protons and neutrons is...

atomic weight

Atomic Mass and Mole Calculations

Atomic mass and mole calculations help explain how much matter is in atoms and compounds. Protons and neutrons have about the same mass, about 1.67 × 10 -24 grams. Scientists define that mass as one atomic mass unit, or amu, also called one Dalton. Electrons are much lighter than protons. They weigh only 9.11 × 10 -28 grams, or about 1/1800 of an atomic mass unit. Because of that small mass, electrons do not add much to an element’s overall atomic mass. When chemists calculate atomic mass,...

isotopes and radioisotopes

Radioisotopes in Medicine and Imaging

Radioisotopes are unstable isotopes that can be used to study the body and treat disease. An isotope is an atom of the same element that has a different mass because it contains a different number of neutrons. It still has the same number of protons, so it remains chemically identical. English chemist Frederick Soddy explained this idea in the early 1900s and later received the Nobel Prize in Chemistry in 1921. Some isotopes have more neutrons than usual and are called heavy isotopes. These...

electron behavior

Electron Shells and Discovery

Electrons are negatively charged subatomic particles that stay near the positively charged nucleus of an atom. They occupy spaces linked to energy levels called shells. They are also arranged into subshells and orbitals within each shell. An electron’s shell shows its general energy level. Electrons closer to the nucleus have less energy, while electrons farther away have more energy. The outer shells have more space, so they can hold more electrons than the inner shells. Subshells describe...

introduction to chemical bonds

How Atoms Bond to Reach Stability

Atoms bond to become more stable, and their outermost electrons play the biggest role in that process. The inner electron shell can hold two electrons. The next two shells can each hold eight electrons. This is called the octet rule. It states that, except for the innermost shell, atoms are most stable when their valence shell, or outer shell, has eight electrons. When atoms do not have enough electrons to fill that outer shell, they form chemical bonds with other atoms. A chemical bond is the...

ionic bonds

Ionic Bonds and Charge Transfer

Ionic bonds form when atoms transfer electrons and become charged particles. A positive ion and a negative ion attract each other because opposite charges pull together. This type of bonding helps explain how some substances are held together. In many cases, an atom loses one or more electrons, while another atom gains them. The atom that loses electrons becomes a cation, which is a positively charged ion. The atom that gains electrons becomes an anion, which is a negatively charged ion. The...

covalent bonds

Polar and Nonpolar Covalent Bonds

Covalent bonds form when atoms share electrons to fill their valence shells. The way those shared electrons are pulled depends on electronegativity, which is an atom's tendency to attract electrons in a bond. That difference also helps explain why some molecules are polar and others are nonpolar. Atoms with similar electronegativities form nonpolar covalent bonds. In these bonds, electrons are shared equally, so there is no charge across the molecule. When two atoms have different...

hydrogen bonds

Hydrogen Bonding and DNA Stability

Hydrogen bonding helps explain why some molecules stick together more strongly than others. A hydrogen bond forms when a weakly positive hydrogen atom, already bonded to an electronegative atom, is attracted to another electronegative atom on a nearby polar molecule. Common examples include water, hydrogen fluoride, and ammonia. This attraction happens because hydrogen has a much lower electronegativity than atoms such as fluorine, oxygen, and nitrogen. The electronegativity difference, along...

ions, molecules, and compounds

Atoms can gain or lose electrons during chemical reactions and become ions. An ion is an atom with an electrical charge. This charge is positive or negative, and it often helps the atom reach a full valence shell. Some atoms are more likely to donate electrons, while others are more likely to accept them. Potassium is one example. It has atomic number 19 and one electron in its valence shell, so it is likely to donate that electron and become a slightly positive ion called a cation. Fluorine...

states of matter

Solids, Liquids, Gases, and Plasma

Solids, liquids, gases, and plasma are the main forms of matter described here. Solids are rigid and keep a definite shape. Liquids flow and take the shape of their container, although gravity gives the surface a flat or slightly curved top. Solids and liquids also have volumes that stay nearly the same even when pressure changes. Gases behave differently from solids and liquids. A gas takes both the shape and the volume of its container. In matter with this behavior, the particles are far...

colloids and suspensions

Suspensions, Sedimentation, and Colloids

Suspensions and colloids are two common kinds of mixtures seen in everyday life. Mud and water, flour and water, and tempera paint are suspensions. These mixtures are heterogeneous, which means their particles are not spread out evenly. The particles are relatively large and can be seen with the naked eye or a magnifying glass. Suspension particles make mixtures cloudy, and they settle out after mixing. The settling of particles in a suspension is called sedimentation. A blood test can measure...

introduction to chemical reactions

Chemical Reaction Basics and Equilibrium

Chemical reactions start with reactants and end with products. Reactants are the substances that enter a reaction, and products are the new substances that form. For example, sodium and chloride ions are the reactants in the formation of table salt. Chemical reactions follow the law of conservation of mass. Matter is not created or destroyed during the reaction. That means the atoms and elements in the reactants are still present in the products, and nothing new appears in the products that...

types of chemical reactions: anabolic and catabolic

types-of-chemical-reactions-anabolic-and-catabolic

Anabolism, Catabolism, and ATP Use

Anabolism and catabolism are the two main kinds of metabolic reactions in the body. Metabolism is the total set of anabolic and catabolic reactions that keep life running. These reactions follow the first law of thermodynamics, which says energy cannot be created or destroyed. It can only change form. Anabolism builds larger, more complex molecules from smaller ones. These anabolic, or biosynthesis, reactions need energy in the form of ATP. They join monosaccharides into polysaccharides, fatty...

types of chemical reactions: exchange and reversible

types-of-chemical-reactions-exchange-and-reversible

Electron Transfer and Chemical Equilibrium

Exchange reactions and reversible reactions are two important ideas in chemistry. In an exchange reaction, synthesis and decomposition happen at the same time. Chemical bonds are both formed and broken. These reactions can absorb chemical energy, store it, and release it. A special type of exchange reaction is the oxidation-reduction reaction, or redox reaction. In a redox reaction, electrons move from one compound to another. The electrons often come from hydrogen atoms, which contain one...

energy transfer in chemical reactions

Chemical Energy and Reaction Types

Chemical reactions depend on energy transfer, chemical bonds, and the way matter collides. A reaction needs enough energy for particles to meet with the right force and precision. That energy can break old bonds and help form new ones. Kinetic energy is the energy of motion. A person lifting a brick uses kinetic energy to move the brick into place on a wall. Once the wall is built, it stores potential energy, which is the energy of position or structure. If the wall falls, that stored energy...

factors influencing the rate of chemical reactions

factors-influencing-the-rate-of-chemical-reactions

Chemical Reaction Rates and Catalysts

Chemical reaction rates depend on how often particles collide and whether those collisions have enough energy to start a reaction. That starting energy is called activation energy. Factors that affect reaction rate either lower that energy or make successful collisions more likely. Concentration and pressure can speed reactions up because they put more particles in the same space. When more particles are present, they are more likely to bump into one another. Chemists can also increase...

acids, bases and neutralization reactions

How pH Affects Cells and Digestion

Acids, bases, and pH help control how cells and body systems work. In biology, pH can strongly affect enzymes, proteins, and nucleic acids. Enzymes work best within a certain pH range, and pH changes can alter their structure or denature them, which changes how they function. Acids release hydrogen ions, or H+, in solution. A hydrogen ion is a proton, so it is very reactive in chemical reactions. Strong acids release all of their H+ in water and ionize completely. Hydrochloric acid (HCl) is a...

key terms and concepts

Learn how atoms become ions, why cations and anions form, and how molecules and compounds differ using potassium, fluorine, oxygen, carbon dioxide, and glucose.

Atomic Charges, Bonds, and Compounds | JoVE K12

anatomy and physiology

JoVE Core 解剖学と生理学では、人体の解剖学的および生理学的な詳細を、包括的で明確で魅力的なビデオ アニメーションで紹介します。このレッスン集は、人体の構造、コンポーネント、機能、要件に焦点を当てています。この知識を実際の医療および研究現場で応用することを実証する科学者による実際のビデオによって補完されています。

Atomic Charges, Bonds, and Compounds

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